Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>Competition Focus>Q 159

HARD

11th CBSE

IMPORTANT

Earn 100

The solubility of a salt of weak acid $(AB)$ at $pH 3$ is $Y x 10^{- 3} mol L^{- 1} .$ The value of $Y$ is _____ (Given that the value of solubility product of $AB$ $(K_{sp}) = 2 x 10^{- 10}$ and the value of ionization constant of $HB (K_{a}) = 1 x 10^{- 8}$ ).

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Important Questions on Ionic Equilibrium in Solution

MEDIUM

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>PROBLEMS FOR PRACTICE>Q 1

Calculate the degree of ionization and

[H_{3} O^{+}]

of

0.01 M {CH}_{3} COOH

solution. The equilibrium constant of acetic acid is

1.8 \times 10^{- 5}

.

HARD

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>PROBLEMS FOR PRACTICE>Q 2

A

0.01 M

solution of acetic acid is

1.34 %

ionised (degree of dissociation

= 0.0134

) at

298 K

. What is the ionization constant of acetic acid?

MEDIUM

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>PROBLEMS FOR PRACTICE>Q 3

What will be the percentage of dissociation in

1.0 M

{CH}_{3} COOH

at equilibrium having dissociation constant of

1.8 \times 10^{- 5}

?

MEDIUM

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>PROBLEMS FOR PRACTICE>Q 4

Nicotinic acid

(K_{a} = 1.4 \times 10^{- 5})

is represented by the formula

HNiC

. Calculate its percentage dissociation in a solution which contains

0.10

mole of nicotinic acid per

2.0

litre of solution.

MEDIUM

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>PROBLEMS FOR PRACTICE

Calculate the concentration of

H^{+}

(aq) in

0 \cdot 2 M

solution of

HCN

. Given that the dissociation constant of

HCN

in water is

4.9 \times 10^{- 10}

.

EASY

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>PROBLEMS FOR PRACTICE

If hydrogen ion concentration in a solution is

1 \times 10^{- 5} moles / litre

, calculate the concentration of

{OH}^{-}

ion in this solution

(K_{w} = 10^{- 14} {moles}^{2} / {litre}^{2})

.

EASY

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>PROBLEMS FOR PRACTICE>Q 1

Calculate the

pH

value of

0.001 N {HNO}_{3}

solution.

EASY

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>PROBLEMS FOR PRACTICE>Q 2

Calculate the

pH

value of

10^{- 3} M HCl

solution.